Concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.24 ×10^-4mol L^-1 solubility product of Ag₂C₂O₄ is_______.

pH of a saturated solution of Ca(OH)₂ is 9. The Solubility product (K_sp) of Ca(OH)₂ _______.

Conjugate base for Bronsted acids H₂O and HF are _______.

Which will make basic buffer?

MY and NY₃, are insoluble salts and have the same K_sp values of 6.2 × 10^-13 at room temperature. Which statement would be true with regard to MY and NY₃?

The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by _______.

With regard to the strength of acids and bases, Find the incorrect statement among the following.

K_w represents _______.

The buffer present in human blood is _______.

The condition for a compound to be precipitated is _______.

 Which among the following is incorrect regarding acids?

Henderson equation for a weak acid and its salt is _______.

An acid is a substance that dissociates to give hydrogen ions in water.
The above concept of acids was proposed by _______.

If ionic product < solubility product then the solution is ________.

The solution whose pH is maintained constant even upon the addition of small amounts of acid or base is called ________.

What are Lewis acids and bases? Give two example for each.

Discuss the Lowry – Bronsted concept of acids and bases.

Indentify the conjugate acid base pair for the following reaction in aqueous solution
i) HS^- (aq) + HF \(\rightleftharpoons \) F^-(aq) + H₂S(aq)
ii) HPO^2-₄ + SO₃^2- \(\rightleftharpoons \) PO₄^3- + HSO₃^-
iii) NH₄⁺ + CO₃^2-  \(\rightleftharpoons \) NH₃ + HCO₃^-

When aqueous ammonia is added to CuSO₄ solution, the solution turns deep blue due to the formation of tetra ammine copper (II) complex,\({ [Cu({ H }_{ 2 }O)_4] }_{ (aq) }^{ 2+ }+ 4{ NH }_{ 3 }(aq)\rightleftharpoons { [Cu{ ({ NH }_{ 3 }) }_{ 4 }] }_{ (aq) }^{ 2+ }\) among H₂O and NH₃ Which is stronger Lewis base.

Define solubility product.

Calculate pH of 10^-7 M HCl

Give the Limitations of Arrhenius concept theory of acids and bases.

What are the two types of buffer? Give an example for each.

How is common ion effect related to the solubility of the electrolyte?

What are the limitations of Ostwald's dilution law?

Explain common ion effect with an example.

Calculate the pH of 1.5\(\times\)10^-3 M solution of Ba(OH)₂

The K_a value for HCN is 10^-9. What is the pH of 0.4M HCN solution?

Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.

 Find the pH of a buffer solution containing 0.20 mole per litre sodium acetate and 0.18 mole per litre acetic acid. K_a for acetic acid is \(1.8\times10^{-5}\).

Based on Arrhenius concept, defame acid and bases and give an example for each.

What do you mean by auto ionisation of water?

How will you calculate solubility product from molar solubility?

What is Henderson equation?

What do you mean by buffer action?

A saturated solution, prepared by dissolving CaF₂(s) in water, has \([Ca^{2+}]=3.3\times10^{-4}M\). What is the K_sp of CaF₂?

K_sp of Al(OH)₃ is 1\(\times\)10^-15M. At what pH does 1.0×10^-3M Al³⁺ precipitate on the addition of buffer of NH₄Cl and NH₄OH solution?

Establish a relationship between the solubility product and molar solubility for the following
a) BaSO₄ 
b) Ag₂(CrO₄)

Calculate the pH of a buffer mixture which contains 7.5 gms if acetic acid and 10.25 gms of sodium acetate in 1 litre of the solution. K_a for acetic acid is 1.8 x 10^-5.

A buffer solution containing 0.1 mole of ammonium hydroxide and 0.15 mole of ammonium chloride per litre of the solution. Calculate the pH of the buffer solution. K_b for ammonium hydroxide is 1.8 x 10^-5.

Explain buffer action in an acidic buffer.

Derive Henderson - Hasselbalch equation